Chemistry -- Acids and Bases

Acids Individual Properties

• Taste sour

• Can sting or burn skin

• React with metals

• Has a pH<7

• Turns blue litmus paper red

Bases Individual Properties

• Taste bitter

• Feel slippery on skin

• Do NOT react with metals

• Has a pH>7

• Turns red litmus paper blue

Both Acids and Bases

• Conduct electricity

• Can neutralize each other

An acidic solution contains

more H+ ions than OH- ions

A basic solution contains

more OH- than H+ ions

When dissolved in water

• Bases produce OH-

• Acids produce H+

Phenolphthalein

• Acids are colorless

• Bright pink in bases

pH

Power of Hydrogen (H+)

All water solutions

contain OH- and H+ ions

Bronsted-Lowry Theory

States that an acid is always a hydrogen ion donor and a base is always a hydrogen ion accepter.

Conjugate Acid

A substance produced when a base accepts an H+ ion, the reaction can be reversed by the conjugate acid donating its H+

Conjugate Base

A substance produced when an acid donates an H+ ion, the reaction can be reversed by the conjugate base accepting an H+

Titration

Procedure to determine the concentration of a solution with a known volume using a solution of known concentration with a burette

Standard Solution

The solution of known concentration

Equivalence Point

When the concentration of H+ from the acid are equal to the concentration of OH- from the base, the solution remains colorless.

End Point

One drop past the equivalence point, the solution is slightly basic so the solution changes to a pink with the phenolphthalein

Neutralization

Concentration of the acid equals the concentration of the base: H+ = OH-

Each increase in one unit of pH is

a 10x decrease in H+ ions (logarithmic)

pH formula

pH = -log[H+]

pH + pOH formula

pH + pOH = 14.00

pOH formula

pOH = -log[OH-]

pOH scale

Power of Hydroxide 14-0

[H+] formula

[H+]=10^-pH

[OH-] formula

[OH-]=10^-pOH